Atomic Structure and Discoveries

<p>Atoms have a dense positive nucleus with electrons orbiting around it. (D)</p> Signup and view all the answers

<p>Emission spectrum (C)</p> Signup and view all the answers

<p>Metals (C)</p> Signup and view all the answers

<p>It gains energy and becomes stable. (C)</p> Signup and view all the answers

<p>Ionization energy (B)</p> Signup and view all the answers

<p>Families (B)</p> Signup and view all the answers

<p>It has the lowest energy and is in the ground state. (B)</p> Signup and view all the answers

<p>The electron emits a photon. (B)</p> Signup and view all the answers

<p>Increases from left to right (D)</p> Signup and view all the answers

<p>They are defined by set paths and energies. (D)</p> Signup and view all the answers

<p>Non-metal (A)</p> Signup and view all the answers

<p>It does not define the exact path of electrons. (B)</p> Signup and view all the answers

<p>He explained atomic spectra using circular electron orbits. (C)</p> Signup and view all the answers

<p>Uncertainty Principle (B)</p> Signup and view all the answers

<p>5 (A)</p> Signup and view all the answers

<p>It loses electrons (C)</p> Signup and view all the answers

<p>1s^2^ 2s^2^ 2p^6^ 3s^2^ (C)</p> Signup and view all the answers

<p>14 (D)</p> Signup and view all the answers

<p>It is said to be isoelectronic (C)</p> Signup and view all the answers

<p>It shows the recurrence of properties of elements (B)</p> Signup and view all the answers

<p>8 (A)</p> Signup and view all the answers

<p>It increases across a period. (C)</p> Signup and view all the answers

<p>An element from group VII A. (A)</p> Signup and view all the answers

<p>Atoms tend to lose, gain, or share electrons for a full set of eight valence electrons. (B)</p> Signup and view all the answers

<p>The number of dots equals the number of valence electrons. (D)</p> Signup and view all the answers

<p>The electronegativity difference is between 0.4 and 1.9. (D)</p> Signup and view all the answers

<p>Group II A (B)</p> Signup and view all the answers

<p>Covalent bond. (D)</p> Signup and view all the answers

<p>Their group number is equal to the number of valence electrons. (C)</p> Signup and view all the answers

<p>The types and number of atoms present (C)</p> Signup and view all the answers

<p>To represent the actual bonding patterns and atom arrangements (C)</p> Signup and view all the answers

<p>Branching carbons should always receive the highest numbers. (B)</p> Signup and view all the answers

<p>Tetra (A)</p> Signup and view all the answers

<p>The carbon atoms with the smallest numbers (A)</p> Signup and view all the answers

<p>The presence of triple bonds (B)</p> Signup and view all the answers

<p>Hepta (C)</p> Signup and view all the answers

<p>Alkene (D)</p> Signup and view all the answers

<p>0.4 or less (B)</p> Signup and view all the answers

<p>16 (C)</p> Signup and view all the answers

<p>2 (D)</p> Signup and view all the answers

<p>Magnesium Nitrate (A)</p> Signup and view all the answers

<p>Mono (C)</p> Signup and view all the answers

<p>Name the metallic element first followed by the nonmetallic element ending in -ide (B)</p> Signup and view all the answers

<p>Equal to 0 (A)</p> Signup and view all the answers

<p>Tetra (A)</p> Signup and view all the answers

Early atomic model. Atoms are positively charged spheres, with negatively charged electrons embedded within.

Atomic model where the atom has a small, dense, positive nucleus with electrons orbiting around it.

Specific colors of light emitted when heated materials or elements are heated.

Model of a hydrogen atom where electrons orbit the nucleus in specific energy levels.

Electron's lowest energy level orbit in an atom.

Electron's higher energy level orbit in an atom.

When an electron moves from a higher energy level to a lower one, it releases a light particle called a photon.

Mathematical model that describes electrons in atoms without defining specific paths.

Arrangement of electrons in different energy levels and sublevels within an atom.

A region surrounding the nucleus where electrons are likely to be found, characterized by a specific energy.

A division within an energy level, further specifying the electron's location.

It's impossible to know both the exact position and momentum of a small particle like an electron at the same time.

Atoms or ions having the same electronic configuration.

Organized arrangement of elements based on increasing atomic number and recurring chemical properties.

Electrons in the outermost energy level of an atom, influencing chemical bonding and reactions.

Number of protons in an atom, also equal to the number of electrons in a neutral atom.

The minimum energy required to remove an electron from a gaseous atom in its ground electronic state.

The change in energy that occurs when an electron is added to a neutral atom in its gaseous state to form a negative ion.

The tendency of an atom to attract electrons towards itself when it is part of a chemical bond.

Atoms tend to gain, lose or share electrons to achieve a stable configuration of eight electrons in their outermost shell.

A diagram that represents valence electrons of an atom as dots surrounding the element's symbol.

A chemical bond formed between two atoms through the electrostatic attraction between oppositely charged ions.

A chemical bond formed between two atoms by sharing electrons.

A type of covalent bond where electrons are unevenly shared due to a difference in electronegativity.

Johann Wolfgang Döbereiner, a German chemist, proposed the Law of Triads in the early 1800s. This law stated that elements could be grouped into sets of three, called triads, based on their similar chemical properties.

John Newlands, a British chemist, proposed the Law of Octaves in 1864. This law suggested that elements with similar properties appeared at regular intervals in the periodic table, repeating every eight elements.

Dmitri Mendeleev, a Russian chemist, published the first widely accepted periodic table in 1869. He organized the elements by increasing atomic mass and noticed that elements with similar properties reappeared periodically.

Henry Moseley, a British physicist, determined the atomic numbers of elements using X-ray spectroscopy in the early 1900s. He realized that the periodic table should be arranged by increasing atomic number, not atomic mass.

The atomic number of an element is the number of protons in the nucleus of an atom of that element. It's a unique identifier for each element.

Valence electrons are the electrons found in the outermost energy level of an atom. These electrons are involved in chemical bonding.

Families or groups are vertical columns in the periodic table. Elements within a family share similar chemical properties due to having the same number of valence electrons.

Periods are horizontal rows in the periodic table. Elements within a period do not necessarily share similar properties, but their properties change gradually across the row.

A type of covalent bond where electrons are shared equally between two atoms with similar electronegativity. This occurs when the difference in electronegativity is 0.4 or less.

A diagram that represents valence electrons of an atom as dots surrounding the element's symbol.

1. Calculate the total available valence electrons (TAVE) in a compound. 2. Calculate the number of electrons required for each atom to achieve a full octet. 3. Subtract TAVE from the octet requirement. 4. Divide this difference by 2 to get the number of bonds.

The system of naming chemical compounds.

Compounds formed from two elements.

Compounds formed from three or more elements, often including a polyatomic ion.

Hydrocarbons where one or more hydrogen atoms are replaced by another element.

Shows the types and number of atoms in a molecule, but not the bonding arrangement.

Shows the actual arrangement of atoms and bonds within a molecule.

Shows all atoms and bonds in a molecule, with all bonds drawn out.

Shorthand formula showing the order of atoms and bonds in a molecule.

A standardized system for naming organic compounds, established by the International Union of Pure and Applied Chemistry.

The longest straight chain of carbon atoms in a molecule.

A group of atoms derived from an alkane by removing one hydrogen atom.